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(C) The principal quantum number $n = 2$ and azimuthal quantum number $l = 1$ corresponds to the $2p$ subshell. For a given $l$,the number of orbitals

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$6$

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(C) The principal quantum number $n = 2$ and azimuthal quantum number $l = 1$ corresponds to the $2p$ subshell. For a given $l$,the number of orbitals is given by $(2l + 1)$. For $l = 1$,the number of orbitals is $2(1) + 1 = 3$. These $3$ orbitals are $p_x, p_y,$ and $p_z$. Each orbital can accommodate a maximum of $2$ electrons. Therefore,the total number of electrons = $3 	imes 2 = 6$.

The total number of electrons that can be accommodated in all the orbitals having principal quantum number $n = 2$ and azimuthal quantum number $l = 1$ is

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